3. What mass of water would need to evaporate from your skin in order to dissipate 1.7X10 J of heat from your body? Given: H2O(1) H2O(g) Hvap = 40.7 kJ/mol or2261 J/g 4. How much energy (heat) is required to convert 52.0 gram of ice at -10.0C to steam at 100 °C? Given: Specific heat (ice): 2.09 J/g•C Htus = 6.02 kJ/mol or 334 J/g Specific heat (water): 4.18 J/g.C Hvap = 40.7 kJ/mol Specific heat (steam): 1.84 J/g-C 5. Acetic acid has a heat of fusion of 10.8 kJ/mol and a heat of vaporization of 24.3 kJ/mol. What is the expected value for the heat of sublimation of acetic acid?
Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
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